Question:

How many of the following have five radial nodes ? 
5s, 6s, 7s, 6p and 4p 

Updated On: Mar 21, 2025
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Correct Answer: 6

Solution and Explanation

Calculation of Radial Nodes: 

The number of radial nodes for an electron in an orbital is given by:

Radial nodes = n - l - 1,

where:

  • n: Principal quantum number
  • l: Azimuthal quantum number

Calculations for the given orbitals:

  • 5s: \(n - l - 1 = 5 - 0 - 1 = 4\) radial nodes
  • 6s: \(n - l - 1 = 6 - 0 - 1 = 5\) radial nodes
  • 7s: \(n - l - 1 = 7 - 0 - 1 = 6\) radial nodes
  • 6p: \(n - l - 1 = 6 - 1 - 1 = 3\) radial nodes
  • 4p: \(n - l - 1 = 4 - 1 - 1 = 1\) radial node

Conclusion:

Only the 6s orbital has five radial nodes. Therefore, the correct answer is 6s.

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Concepts Used:

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  • P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
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